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It depends on how many clouds of lone electrons (electrons that aren't participating in bonds) there are. When looking at the molecular geometry is really important to count ALL electron clouds. There are two types of these, the electrons that are participating in bonding and the lone pairs of electrons. A molecule or compound that has tetrahedral geometry has 4 electron clouds, all participating in bonding. Since all the four bonds are identical it forms a tetrahedron which is the shape that allows for all bonds to be the same. A molecule that has square planar geometry does NOT have 4 electron clouds. In fact, it has 6 electron clouds, four of them participating in bonding and the other two are lone pair of electrons. The lone pairs have the most steric hindrance out of all the electron clouds. Because of this, the lone pairs of electrons positions themselves exactly above and below the molecule and the 4 remaining bonds have to position themselves on the "equator" of the molecule. This makes the four bonds form a square in the middle of the molecule and this is what we see. Hope this helps.
1:25 how do you know whether the compound is ligand just by looking at the equation.....also sir for 8:05 as the charge increases, isn't the coordination number generally decreasing? for 10:07 why did you have to draw zinc when carbon is already bonded with two oxygen atoms [or ions].......11:42 i do not see chromium having 3 atoms of it
Ligands are the groups bonded to the metal ion, so in Zn(H2O)6 2+ there are 6 H2O ligands bonded to Zn 2+ For coordination number you need to look at that data again. But it's only a general rule, you'll find transition metals form many different complexes. He's drawing the bonds between the oxalate ion and the zinc metal... He didn't say there's 3 atoms of Cr, look at the formula, he's saying it has a +3 charge because of the 3 x CN- counter ions. Based on your questions I think you should watch this one again and maybe check out some other transition metal videos too.
In most part of the video, you kept saying that coordination number is the number of ligands attached but it's somewhat an incorrect definition, y'know. Coordination number depends on the number of dative bonds central metal ion is attached to, so let's say if a hexadentate ligand (a molecule or ion that can form six dative bonds) attaches itself with a transition metal ion, it's coordination number will be six depending on what I said and would be one from what you have explained, which would be wrong.
@@amnanavid well, in our book, the definition is given that any d block metal that forms any ion which has 1-9 e- in its d orbital. but Zn doesn't seem to comply to that,so I said so
I might not have time to look at the video right now (will do later) but I was wondering why the metal within complex ions was drawn with dashed bonds and the ligants still had their electron pairs draw right between the bond and the atom? Is it related to resonance form in any way or are the bonds just conventionally drawn that way? I have to ''discuss'' the metal's geometry in EDTA-Ca^2- for a lab report, it obviously looks like an octahedron but you never know.
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why does the 2 go at the end? Is that Algebra? pemdas? or what?
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yeah...if uploading a good video clarify the Nobel peace distribution standards ...then why not.....let's stop the Nobel recipients from working their asses off and suggest them to upload TH-cam videos😎😎
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i am phd physics student who has no idea about coordination chemistry nut they asked me to pass this course and i was totally lost
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InfiniteLoop they’re a PhD student, meaning it’s been years since they’ve been in high school let alone do high school chemistry content.
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at 11:52, shouldn't you have bracketed the (CN) at the top so it looks like (CN)3? otherwise it looks like 1 carbon and 3 nitrogens.
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how do i tell when to use a tetrahedral or a square planar since those are the two options for a coordination number of 4?
I thought there's no lone pairs for the tetrahedral complex, but I'm probably wrong.
depends of the ligand structure i think.
It depends on how many clouds of lone electrons (electrons that aren't participating in bonds) there are. When looking at the molecular geometry is really important to count ALL electron clouds. There are two types of these, the electrons that are participating in bonding and the lone pairs of electrons.
A molecule or compound that has tetrahedral geometry has 4 electron clouds, all participating in bonding. Since all the four bonds are identical it forms a tetrahedron which is the shape that allows for all bonds to be the same.
A molecule that has square planar geometry does NOT have 4 electron clouds. In fact, it has 6 electron clouds, four of them participating in bonding and the other two are lone pair of electrons. The lone pairs have the most steric hindrance out of all the electron clouds. Because of this, the lone pairs of electrons positions themselves exactly above and below the molecule and the 4 remaining bonds have to position themselves on the "equator" of the molecule. This makes the four bonds form a square in the middle of the molecule and this is what we see.
Hope this helps.
fruitloops It depends on how many lone pairs are on the metal
If it’s sp3 (or d3s) => tetrahedral. If it’s dsp2 => sqare planar. You basically need to do the hybridation of the metal
Great explanations, thank you!!
1:25 how do you know whether the compound is ligand just by looking at the equation.....also sir for 8:05 as the charge increases, isn't the coordination number generally decreasing? for 10:07 why did you have to draw zinc when carbon is already bonded with two oxygen atoms [or ions].......11:42 i do not see chromium having 3 atoms of it
Ligands are the groups bonded to the metal ion, so in Zn(H2O)6 2+ there are 6 H2O ligands bonded to Zn 2+
For coordination number you need to look at that data again. But it's only a general rule, you'll find transition metals form many different complexes.
He's drawing the bonds between the oxalate ion and the zinc metal...
He didn't say there's 3 atoms of Cr, look at the formula, he's saying it has a +3 charge because of the 3 x CN- counter ions.
Based on your questions I think you should watch this one again and maybe check out some other transition metal videos too.
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In most part of the video, you kept saying that coordination number is the number of ligands attached but it's somewhat an incorrect definition, y'know. Coordination number depends on the number of dative bonds central metal ion is attached to, so let's say if a hexadentate ligand (a molecule or ion that can form six dative bonds) attaches itself with a transition metal ion, it's coordination number will be six depending on what I said and would be one from what you have explained, which would be wrong.
Please do a video on activation complex
Great video
Do u have anything on Fac-mer isomers? They are in the same chapter as this one. Thanks
6:18 this is where i get a bit confused. What dictates Td or D4h shapes
do we have to memorise the coordination number of each ion? I don't get how he got them from 6:55. Someone please help
Sir,pls tell me that, how can I identify the situation of the ligand in complex compound??? Is it cation ,anion or neutral???
You have to add the charges from each ion, if total charge is +ve, cation, if -ve, anion and if total charge 0, it is neutral
thanks for the great job and please can you make a video for order of reactions??
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hey! when you talk about bidentates, you use zinc ion as an example. Zinc ion can not form a complex ion as it has a complete 3-d orbital....
Sir can you say when the NO3 acts as counter ion
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u should make a video on chelating effect
But zinc is not a transition metal, but why do we calculate the coordination number in this case.
Zinc IS a transition metal it is just ‘non-typical’ transition metal
@@amnanavid well, in our book, the definition is given that any d block metal that forms any ion which has 1-9 e- in its d orbital. but Zn doesn't seem to comply to that,so I said so
Thanks alot🎉
I might not have time to look at the video right now (will do later) but I was wondering why the metal within complex ions was drawn with dashed bonds and the ligants still had their electron pairs draw right between the bond and the atom? Is it related to resonance form in any way or are the bonds just conventionally drawn that way? I have to ''discuss'' the metal's geometry in EDTA-Ca^2- for a lab report, it obviously looks like an octahedron but you never know.
Oh nevermind, it was just coordinate covalent bonds, I had no clue lol
Helpful sir
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Is there a playlist for coordination chemistry?
Plz make vedio of differential equation solved some board problem also ..
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Thank you